The Periodic Table - KING'S SCIENCE...
Transcript of The Periodic Table - KING'S SCIENCE...
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The Periodic Table
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The Big Questions
Who developed the first modern periodic table?
How did he organize it, and how does this differ from the organization of the P. T. today?
What are some ways in which we group elements on the P. T.?
What does this tell us about the atom’s structure?
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The First Modern P. T.
Developed in 1869 by Dmitri Mendeleev.
Russian chemist and inventor.
Arranged elements according to inc. atomic mass
and periodicity.
Periodicity – tendency of elements to repeat
properties.
Example: Lithium is a metal that reacts explosively
with H2O.
This property is repeated in Na, then again in K, and
so on...
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Dmitri Ivanovich Mendeleev
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The First Modern Periodic Table
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The First Modern P. T.
DM noticed there were “holes” where no
known element would fit.
Guessed that these holes represented
undiscovered elements.
Made predictions about their properties.
When discovered, these elements matched
their predicted properties.
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Periods (Rows)
Periods – horizontal rows of elements.
All elements on a period have the same
number of energy levels.
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Periods
How many energy levels would you expect to find in atoms
from the 4th row? The 5th row?
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Families of Elements
Families – columns or groups.
Elements in a family have similar chem.
properties.
Also have same no. of valence e-.
Coincidence? (No.)
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Ions
Atoms can lose or gain electrons.
Ion – an atom that has become charged by
gaining or losing electrons.
Cation – positive ion (lost e-)
Anion – negative ion (gained e-)
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Ions
Gain 1 e-
C-
6 p+
7 e-
C
6 p+
6 e-
Lose 1 e-
C+
6 p+
5 e-
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The Octet Rule
Atoms tend to gain or lose electrons so
they can have 8* valence electrons (same e-
configuration as a noble gas).
Why?
8 valence electrons = full s and p sublevel.
Extremely stable configuration.
*There are a few exceptions to this rule that
we will discuss later.
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Families of the Periodic Table
Group 1A (1)
Alkali metals
1 val. e-
Form +1 ions.
Group 2A (2)
Alkaline earth metals
2 val. e-
Form +2 ions.
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Families of the Periodic Table
Groups 3B – 2B (3 – 12)
Transition metals
Have variable val. e-
Can form multiple cations.
Group 3A (13)
Boron group
3 val. e-
Form +3 ions.
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Families of the Periodic Table
Group 4A (14)
Carbon group
4 val. e-
C and Si rarely form ions. All others: +2 or +4
Group 5A (15)
Nitrogen group
5 val. e-
Form –3 ions (except for bismuth: +3)
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Families of the Periodic Table
Group 6A (16)
Chalcogens
6 val. e-
Form –2 ions.
Group 7A (17)
Halogens
7 val. e-
Form –1 ions.
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Families of the Periodic Table
Group 8A (18)
Noble gases
8 val. e- (exc. He)
Do not form ions.
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Blockss-
blo
ck
p-blockd-block
f-block
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Metals, Metalloids, and Nonmetals
Metals
Majority of elements are metals
Conductors of heat and electricity.
Lose electrons (form + ions).
Nonmetals
About 16 elements.
Insulators.
Tend to gain or share e-
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Metals, Metalloids, and Nonmetals
Metalloids
Between metals and nonmetals.
Semi-conductors.
Lose or share electrons.
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Metals, Metalloids, and Nonmetals
Metals
Metalloids
Nonmetals
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Metallicity
More Metallic Less Metallic
Mo
re M
etall
icL
ess
Met
all
ic
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Electron Configs. on the P. T.
1s
2s
3s
4s
5s
6s
7s
3d
4d
5d
6d
4p
5p
6p
7p
3p
2p
1s
4f
5f